Do you really use up all of the limiting reagent?

Write down the equation that you would have to solve in order to get the concentration of each type of molecule at equilibrium. (Hint: plug the data from the table into the equilibrium constant expression.)

Use the applet to find the value of "x" that is the solution to your problem.

Now you know that when you put 8 moles of N2 and 5 moles of H2 into the reaction chamber that the solution to the problem is x = 1.17. That is, if you worked the problem by hand using the equilibrium table that you saw in class, this is the answer that you should get.

 

In the probelm that you just did (8 moles N2 and 5 moles of H2 initially), what was the limiting reagent?
N2
H2
NH3
There is no limiting reagent


What is the concentration of H2 at equilibrium?

Did all of the limiting reagent react in this problem?
Yes
No
Is there any combination of H2, H2 and H3 that you can put in the reaction champer and get all of the limiting reagent ot react?
Yes
No

 

Back to Concepts and Problems to Work